Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of
the partial pressures of each of the individual gases.
What is the partial pressure of xenon if the total
pressure of the mixture is 7.524 atm and the mixture
contains xenon, 3.78 atm argon and 1.46 atm of neon?

ch3 [ch2]14cooh

explanation:

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)